Question

Write balanced chemical equations for the reaction of hydrogen gas with oxygen, chlorine, and nitrogen.

Short answer

The balanced equations are: \( 2H_2 + O_2 \rightarrow 2H_2O \), \( H_2 + Cl_2 \rightarrow 2HCl \), and \( 3H_2 + N_2 \rightarrow 2NH_3 \).

Step-by-step solution

Write the Chemical Formulas

First, write the chemical formulas for each element involved in the reactions. Hydrogen gas is written as \( H_2 \), oxygen as \( O_2 \), chlorine as \( Cl_2 \), and nitrogen as \( N_2 \).

Hydrogen and Oxygen Reaction

Combine \( H_2 \) with \( O_2 \) to form water \( H_2O \). The unbalanced equation: \( H_2 + O_2 \rightarrow H_2O \).

Balance Hydrogen and Oxygen Equation

To balance \( H_2 + O_2 \rightarrow H_2O \), ensure atoms of each type are equal on both sides. Use coefficients: \( 2H_2 + O_2 \rightarrow 2H_2O \).

Hydrogen and Chlorine Reaction

Combine \( H_2 \) with \( Cl_2 \) to form hydrochloric acid \( HCl \). The initial equation is: \( H_2 + Cl_2 \rightarrow HCl \).

Balance Hydrogen and Chlorine Equation

Ensure the number of each type of atom is the same on both sides: \( H_2 + Cl_2 \rightarrow 2HCl \).

Hydrogen and Nitrogen Reaction

Combine \( H_2 \) with \( N_2 \) to form ammonia \( NH_3 \). The unbalanced equation: \( H_2 + N_2 \rightarrow NH_3 \).

Balance Hydrogen and Nitrogen Equation

To balance \( H_2 + N_2 \rightarrow NH_3 \), find coefficients that equalize each atom: \( 3H_2 + N_2 \rightarrow 2NH_3 \).

Review All Balanced Equations

Check the balanced equations: \( 2H_2 + O_2 \rightarrow 2H_2O \), \( H_2 + Cl_2 \rightarrow 2HCl \), and \( 3H_2 + N_2 \rightarrow 2NH_3 \).

Key concepts

Chemical Reactions

Chemical reactions are processes where substances, known as reactants, transform into different substances, referred to as products. This occurs through the breaking and forming of bonds between atoms. Each reaction involves a change in chemical composition, which can often be represented using a chemical equation. In these equations, reactants are listed on the left side, and products on the right, separated by an arrow indicating the direction of the reaction.

Understanding chemical reactions involves recognizing the types of reactions and the patterns they follow. For instance, synthesis reactions involve combining simpler substances into a more complex compound. In our original exercise, we have synthesis reactions where hydrogen gas reacts with oxygen, chlorine, and nitrogen to form water, hydrochloric acid, and ammonia respectively.

Each of these reactions illustrates how molecules interact: hydrogen shares its electrons with oxygen in water, with chlorine in hydrochloric acid, and with nitrogen in ammonia. The transformation from reactants to products helps understand energy changes and the conservation of mass in reactions, as no atoms are lost or gained, just rearranged.

Stoichiometry

Stoichiometry is the study of the quantitative relationships in chemical reactions. It allows chemists to predict the proportions of reactants needed and products formed in a given reaction. Stoichiometry is at the heart of balancing chemical equations, ensuring that the same number of each type of atom appears on both sides of a reaction equation.

When balancing a chemical equation, stoichiometry is used to determine the correct coefficients for each reactant and product. Coefficients are numbers placed in front of compounds to indicate their ratios in a balanced equation. For instance, in the reaction between hydrogen and oxygen to form water, the stoichiometric coefficients are 2 for hydrogen and 1 for oxygen, with 2 for water. This means two molecules of hydrogen react with one molecule of oxygen to produce two molecules of water.

To apply stoichiometry effectively, you need to understand the law of conservation of mass, which states that mass in an isolated system is neither created nor destroyed by chemical reactions. This principle ensures the mass of the reactants equals the mass of the products, reflecting the balancing act required in every chemical equation.

Chemical Formulas

Chemical formulas are a shorthand representation of the types and numbers of atoms in a substance. They are essential in describing the composition of molecules and compounds. Understanding how to write and interpret chemical formulas is crucial in studying chemical reactions.

A chemical formula uses symbols from the periodic table with subscripts to denote the number of atoms. For example, the formula for water is \( H_2O \), which indicates it contains two hydrogen atoms and one oxygen atom. In the original exercise, hydrogen gas is written as \( H_2 \), indicating two hydrogen atoms bonded together, and oxygen as \( O_2 \), chlorine as \( Cl_2 \), each representing diatomic molecules, common for gases in their natural state.

Correctly using chemical formulas allows you to graphically depict the reactants and products in a chemical reaction equation. They are vital for understanding the material's properties and predicting how it might interact with others in a reaction. The chemical formulas provide a clear and succinct method to detail every reaction component, which facilitates balancing the equation according to the laws of stoichiometry.